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olchik [2.2K]
3 years ago
5

Which is bigger mL or quarts

Chemistry
2 answers:
VLD [36.1K]3 years ago
7 0
A quart is bigger because 1 quart= 946.353 ml. I hope this helps. :)<span />
Nataly [62]3 years ago
5 0
 Your answer would be Quarts .
You might be interested in
Se ha añadido un evaporador para una alimentación de 11500 kg/dia de zumo de pomelo de forma que evapore 3000 kg/dia de agua por
mamaluj [8]

Answer:

37 %.

Explanation:

¡Hola!

En este caso, para el problema descrito, conocemos la corriente de entrada y la de salida del agua, por lo que podemos obtener el flujo de la corriente que contiene el zumo a la salida una vez el agua fue evaporada:

F_{sol}=11500kg/dia-3000kg/dia=8500 kg/dia

Luego, por medio de un balance de zumo de limón en el evaporador en el cual la cantidad que entra es igual a la que sale con sus respectivas concentraciones:

x_z^{entra}*11500kg/dia=x_z^{sale}*8500kg/dia

Como la concentración del zumo a la salida es del 50 % (0.50), la de entrada es:

x_z^{entra}=\frac{x_z^{sale}*8500kg/dia}{11500kg/dia} =\frac{0.50*8500kg/dia}{11500 kg/dia}\\ \\x_z^{entra}=0.37

Que es igual al 37%.

¡Saludos!

6 0
3 years ago
How many grams of KBr is required to prepare 100 mL of<br> 2.0 M KBr solution?
sesenic [268]

Answer:

23.8g

Explanation :

Convert 2.0M into mol using mol= concentration x volume

2.0M x 0.1L (convert 100mL to L since the units for M is mol/L)

= 0.2 mol

We can now find grams by using the molar mass of KBr

=119.023 g/mol (Found online) webqc.org

but can be be calculated by using the molecular weight of K and Br found on the periodic table

We can now calculate the grams by using grams=mol x molar mass

119.023g/mol x 0.2mol

= 23.8046 g

=23.8g (rounded to 1decimal place)

4 0
2 years ago
Kool-Aid is made up of sugar (C6H12O6), food coloring, and water. It is an example of a(n)
ololo11 [35]
I think it’s compounds
3 0
3 years ago
Read 2 more answers
WILL MARK YOU THE BRAINLIEST IF YOU ANSWER THESE TWO QUESTION CORRECTLY :)
lara [203]

Answer: 1. HYDROCARBONS? 2. ALKANES?

i'm not exactly AMAZING at this but i did some research and this is what i think it is i'm also not in this grade but i tried.

7 0
3 years ago
A sample of gas has a density of 0.53 g/L at 225 K and under a pressure of 108.8 kPa. Find the density of the gas at 345 K under
sukhopar [10]

Answer:

\rho _2=0.22g/L

Explanation:

Hello!

In this case, since we are considering an gas, which can be considered as idea, we can write the ideal gas equation in order to write it in terms of density rather than moles and volume:

PV=nRT\\\\PV=\frac{m}{MM} RT\\\\P*MM=\frac{m}{V} RT\\\\P*MM=\rho RT

Whereas MM is the molar mass of the gas. Now, since we can identify the initial and final states, we can cancel out R and MM since they remain the same:

\frac{P_1*MM}{P_2*MM} =\frac{\rho _1RT_1}{\rho _2RT_2} \\\\\frac{P_1}{P_2} =\frac{\rho _1T_1}{\rho _2T_2}

It means we can compute the final density as shown below:

\rho _2=\frac{\rho _1T_1P_2}{P_1T_2}

Now, we plug in to obtain:

\rho _2=\frac{0.53g/L*225K*68.3kPa}{345K*108.8kPa}\\\\\rho _2=0.22g/L

Regards!

8 0
3 years ago
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